A 1.00 molar .aqueous solution of trichloroacetic acid ("CCl"_(3)"COOH") is heated to its boiling point. The solution has the boiling point of 100.18 ""^(@)C. Determine the Van't Hoff factor for trichloroacetic acid. (K_(b) "for water" = 0.512 "kg mol"^(-1)).

A 1.00 molar .aqueous solution of trichloroacetic acid ("CCl"_(3)"COOH

1.	A 1.00 molar .aqueous solution of trichloroacetic acid ("CCl"_(3)"COOH") is heated to its boiling point. The solution has the boiling point of 100.18 ""^(@)C. Determine the Van't Hoff factor for trichloroacetic acid. (K_(b) "for water" = 0.512 "kg mol"^(-1)).
Answer» SOLUTION :`DELTA T_(b) = iK_(b)`m `(100.18 - 100)^(@)C = I XX 0.512 k" mol"^(-1) xx 1 ` m 0.18 K = i`xx 0.512` K g `mol^(-1) xx 1` m i= 0.35 OR (i) Mole fraction is the ratio of number of moles of one component to the total number of moles in a mixture.`"" `[ Or mathematical expression ] `x_(A) = (n_(A))/(n_(A) + n_(B))` Where `n_(A)`= number of moles of component A. `n_(B)` = number of moles of component B. (ii) Solution which obey Raoult.s law over the ENTIRE range of concentration are called ideal solutions.